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Assertion: Nitrogen has higher ionizatio...

Assertion: Nitrogen has higher ionization enthalpy than oxygen.
.Reason: Oxygen has stable half filled configuration .

A

Assertion and reason both are correct statements and reason is correct explanation for assertion.

B

Assertion and reason both are correct statements but reason is not correct explanation for assertion.

C

Assertion is correct statement but reason is wrong statement.

D

Assertion is wrong statement but reason is correct statement.

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the given assertion and reason, we will follow these steps: ### Step 1: Understand the Assertion The assertion states that "Nitrogen has higher ionization enthalpy than oxygen." **Explanation**: - Ionization enthalpy (or ionization energy) is the energy required to remove an electron from an atom in its gaseous state. - We need to compare the ionization enthalpy of nitrogen (N) and oxygen (O). ### Step 2: Determine the Electron Configurations - The electron configuration of nitrogen (atomic number 7) is: - \(1s^2 2s^2 2p^3\) - The electron configuration of oxygen (atomic number 8) is: - \(1s^2 2s^2 2p^4\) ### Step 3: Analyze the Stability of the Electron Configurations - Nitrogen has a half-filled p orbital configuration (2p^3), which is known to be more stable due to symmetry and exchange energy. - Oxygen has a p orbital configuration of 2p^4, which is not half-filled. ### Step 4: Compare Ionization Energies - Generally, atoms with half-filled or fully filled orbitals are more stable and require more energy to remove an electron. - Therefore, nitrogen, with its half-filled p orbital, will have a higher ionization enthalpy compared to oxygen. ### Step 5: Evaluate the Reason The reason states that "Oxygen has a stable half-filled configuration." - This statement is incorrect because oxygen does not have a half-filled configuration; nitrogen does. ### Conclusion - The assertion is **true**: Nitrogen has a higher ionization enthalpy than oxygen. - The reason is **false**: Oxygen does not have a stable half-filled configuration. ### Final Answer - Assertion: True - Reason: False
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Knowledge Check

  • Assertion Nitrogen has higher first ionisation energy than oxygen. Reason Atomic radius of nitrogen is smaller than that of oxygen.

    A
    Both Assertion and Reason are correct and Reason is the correct explanation on the Assertion.
    B
    Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
    C
    Assertion is correct but Reason is incorrect
    D
    Assertion is incorrect but Reason is correct

  • Atomic nitrogen has a higher ionization energy than atomic oxygen. This is best explained by:

    A
    by lower electron-electron repulsion in nitrogen
    B
    the greater effective nuclear charge of nitrogen
    C
    the fact that the electron ionized in N is from the 2s subshell, while that ionized from O is from the 2p subshell
    D
    the fact that N has an odd number of electron while O has an even number.

  • Beryllium has higher ionisation enthalpy than boron.This can be explained as,

    A
    Beryllium has higher size than boron hence its ionisation enthalpy is higher
    B
    Penetration of 2p-electrons to the nucleus is more than the 2s-electrons
    C
    It is easier to remove electron from 2p-orbital as compared to 2s-orbital due to more penetration of s-electrons
    D
    Ionisation energy increases in a period.

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